Add your answer and earn points. A) 5 moles of O2 produce 4 moles of NO. Solution for Consider the reaction: NH3 + O2 → NO + H2O For every 150 g NH3, Find the mass of NO produced. The first thing you need is a balanced equation for the reaction: 4 NH3 + 5 O2 → 4 NO + 6 H2O. The balanced reaction is: 4NH3 + 5O2 --> 4NO + 6H2O. And the answer would be 4.78 x 4/5 or 3.824 moles of NO. So the conversion factor would be 4/5. This would produce 8.0 moles of NO. Find the mass of H2O produced. Which reactant is the limiting reagent?… ash1719 ash1719 Redox and neutralization reaction Still have questions? 1. Problem: NH3 + O2 → NO + H2O (Unbalanced)If at the beginning of the reaction you used 6.89 g NH3 and 15.76 g O2, what is the theoretical yield (in grams) of NO (you will need to find the limiting reagent and then the theoretical yield of NO from this reagent)? In an experiment, 3.25g of NH3 are allowed - 16235523 Still have questions? For the reaction NH3 + O2 --> NO + H2O how many grams of O2 are needed to completely react with 85.15 g of NH3 ? In an experiment 3.25g of NH3 are allowed to react with 3.50g of O2. 160.00 g / 16.00 g/mol = 10.0 moles of O2. Find more answers. Solution for Take the reaction: NH3+O2-> NO+H2O. Both of them limit the Hydrogen. 160.00 g of O2 / g/mol for O2 = number of moles of O2. Remember the moles of the unknown is in the numerator. Limiting reactant is Nitrogen and Oxygen, by just giving it a quick look. So the molar ration is 5 to 4. You need more information to answer the next two, as … Molar Mass:… 8.0 moles * 30.01 g/mol = 240.08 grams of Nitric oxide. Identify the type of reaction NH3+O2---> NO + H2O 1 See answer apoorvavishwasr4476 is waiting for your help. First you have to balance the reaction to determine the mole ratios of the reactants and products. Take the reaction: NH3 + O2 + NO + H2O. A. Ask your question.